Acid–base
Acid–base reaction is a chemical reaction that occurs between an acid and a base. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Bronsted–Lowry acid–base theory.
Definition[edit | edit source]
An acid–base reaction is a type of chemical process typified by the exchange of one or more hydrogen ions, H+, between species that may be neutral (molecules, such as water, H2O) or electrically charged (ions, such as ammonium, NH4+; hydroxide, OH−; or carbonate, CO32−).
Acid–base theories[edit | edit source]
The first scientific concept of acids and bases was provided by Lavoisier in around 1776. Since Lavoisier's knowledge of strong acids was mainly restricted to oxygen-containing acids, such as H2SO4 (sulfuric acid) and H2CO3 (carbonic acid), he defined acids in terms of their containing oxygen, which in fact he named from Greek words meaning "acid-former" (from the Greek οξυς (oxys) meaning "acid" or "sharp" and γεινομαι (geinomai) meaning "engender"). The Lavoisier definition was replaced by the Brønsted–Lowry acid–base theory, the Arrhenius acid and the Lewis acid definitions.
Brønsted–Lowry theory[edit | edit source]
The Brønsted–Lowry theory is an acid–base concept, introduced independently by Johannes Nicolaus Brønsted and Thomas Martin Lowry in 1923. In this system, an acid and a base are defined respectively as a proton (hydrogen ion, H+) donor and acceptor.
Lewis theory[edit | edit source]
The Lewis theory was first proposed by Gilbert N. Lewis in 1923. In the Lewis theory, an acid is an electron pair acceptor and a base is an electron pair donor.
Applications[edit | edit source]
Acid–base reactions are essential in both biochemistry and industrial chemistry. Moreover, many of the substances we encounter in our homes, the supermarket, and the pharmacy are acids or bases.
See also[edit | edit source]
References[edit | edit source]
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